CH 3 - notes 5 - elemental analysis
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CH 3 - notes 5 - elemental analysis

Course Number: CHEM 1110, Fall 2011

College/University: St. Johns

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AP chem.. OMalley Text: p 91 96 (3.6) Chapter 3 stoichiometry 4 (elemental analysis) Name: ____________________ ELEMENTAL ANALYSIS EX 0.1156 g CxHyNZ reacts with O2 to give 0.1638 g CO2, 0.1676 g H2O, and N2. Find the empirical formula. CxHyNz + O2 CO2 + H2O + N2 3.79 Cumene is a compound containing only carbon and hydrogen that is used in the production of acetone and phenol in the chemical industry....

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chem.. AP OMalley Text: p 91 96 (3.6) Chapter 3 stoichiometry 4 (elemental analysis) Name: ____________________ ELEMENTAL ANALYSIS EX 0.1156 g CxHyNZ reacts with O2 to give 0.1638 g CO2, 0.1676 g H2O, and N2. Find the empirical formula. CxHyNz + O2 CO2 + H2O + N2 3.79 Cumene is a compound containing only carbon and hydrogen that is used in the production of acetone and phenol in the chemical industry. Combustion of 47.6 mg cumene produces some CO 2 and 42.8 mg water. The molar mass of cumene is between 115 and 125 g/mol. Deter mine the empirical and molecular formulas of cumene. S. OMalley 2011 HOMEWORK (CH 3 part 5) 3.71 There are two binary compounds of mercury and oxygen. Heating either of them results in the decomposition of the compound, with oxygen gas escaping into the atmosphere and a residue of pure mercury remaining. Heating 0.6498 g of one of the compounds leaves a residue of 0.6018 g. Heating 0.4172 g of the other compound results in a mass loss of 0.016 g. Determine the empirical formula of compound. 3.117 each A sample of LSD (D-lysergic acid diethylamide, C24H30N3O) is added to some table salt (sodium chloride) to form a mixture. Given that a 1.00 g sample of the mixture undergoes combustion to produce 1.20 g of CO 2, what is the mass percentage of LSD in the mixture? (CHALLENGE) 3.131 Consider a gaseous binary compound with a molar mass of 62.09 g/mol. When 1.39 g of this compound is completely burned in excess oxygen, 1.21 g of water is formed. Determine the formula of the compound. Assume water is the only product that contains hydrogen (CHALLENGE) 3.143 An ionic compound MX3 is prepared according to the following unbalanced chemical equation: M + X2 MX3 20 A 0.105 g sample of X2 contains 8.92 x 10 molecules. The compound MX3 consists of 54.47% X by mass. W hat are the identities of M and X, and what is the correct name for MX 3? Problems taken from Zumdahl, 7th ed. 3.71 compound I: HgO; compound II: Hg2O 3.79 C3H4; C9H12 3.117 42.8% 3.131 N4H6 3.143 M = Y, X = Cl, YCl3, yttrium(III) chloride

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